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A Chemistry Chapter 11 Study Guide
1. periodic table                               8. valence electron
2. periodic law                                 9. core electrons
3. first ionization energy                   10. inert
4. group                                          11. isoelectronic
5. family                                          12. periodic trends
6. periods                                        13. atomic radius
7. series                                           14. shielding

1. What was Mendeleev’s contribution to the science of Chemistry?
2. Explain how Mendeleev arranged the elements.
3. How is today’s periodic table different from Mendeleev’s?
4. Why is Group 1 known as “alkali metals”?
5. Draw a periodic table. Label alkali metals, alkaline earth, halogens, noble gases, representative elements, transition metals, inner-transition metals, lanthanide series, actinide series, nonmetals, metalloids.
6. Compare the group number of the representative elements to the number of valence electrons.
7. Describe the reactivity of an atom in which the valence orbital is full.
8. Compare metals and nonmetals with regard to their tendency to gain or lose electrons. How many will they generally gain or lose?
9. How are transition metals different from representative elements?
10. How does atomic radii change in a period? In a group? Why?
11. Compare the size of a cation or anion to its neutral ‘parent’ atom.
12. What are the general trends for ionization energies across the periodic table and down a group of the periodic table? Explain any deviations.
13. Describe the size of successive ionization energies.
14. Review Fig. 11-9 on page 385.

p. 368 3,4
p. 375 7,8
p.377 11,12,13,14,15,16,17
p. 385 20,22
Review 10,11,12,13,14,15,16,18,19,20,22,23,24,27,28,29,30,36,38,41,44,45,46,47,48,